A)Under standard conditions , will the oxidation of lactate using Fe3+ as electron acceptor prove energetically favorable? What is the change in free energy associated with the complete oxidation of lactate to carbon dioxide by Fe3+? (Assume reduction of Fe3+ to Fe2+) Given information pe0=-0.68 (My knowledge about this is: p
Can you please assist me in understanding what the name of the products and the net ionic equations are for the following mixtures? -ammonia poured into aluminum nitrate -barium chloride poured into sodium sulfate -copper(II) chloride poured into sodium carbonate -lead(II) nitrate poured into potassium iodide -m
The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate and citric acid 3 NaHCO3 + H3C6H5O7 --> 3 CO2 + 3 H2O + Na3C6H5O7. In a certain experiment 1.20g of sodium bicarbonate and 1.20g of citric acid are allowed to react. Which is the limiting reactant?
If we were to add sodium carbonate and calcium carbonate to separate samples of Al2(SO4)3, what would the reaction/equilibrium equations look like? What are the pKa values of Na2SO4 and CaSO4 ---- even though they are salts, would they continue to add at least in part to the acidity of the solution?
A) Balance the following equations. b) Determine the by-products of each reaction. c) Select the most preferred base to use in balancing the equation. d) Quote the pKb for each base used. The preference for the ultimately selected base is to be determined by: a) which would be the safest base to handle, b) which produce
1. Write the balanced equation for the first step in the reaction between vinegar and baking soda, with carbonic acid (H2CO3) as a product. What type of reaction is this? 2. Write the balanced equation for the second step in the reaction, the liberation of carbon dioxide from carbonic acid. What type of reaction is this? 3
example 1: A solution is prepared by adding 0.1 Mol of sodium sulfide, Na2S, to 1.00 L of water. The solution is: - basic - neutral - acidic example 2: A solution is prepared by adding 0.1 Mol of lithium nitrate LiNO3, to 1.00 L of water. The solution is: - basic - neutral - acidic
Hydrofluoric acid (HF) has an equilibrium constant Ka value of 7.2 x 10^- 4. Part a: 0.250 mol of F-- ions (in the form of NaF) are added to 1.0 Liters of 0.1 mol L-1 aqueous HF. Calculate the resulting pH? Part b: The solution produced in (part a) is added 10.0 ml of 5.0 mol L-1 NaOH. Calculate the resulting PH?
5. 0.1060g of sodium carbonate, dissolved in 20ml of water, was expected to give a titre of approximately 20ml of hydrochloric acid. what would you expect the approximate titre value to be if the carbonate had been dissolved in 40ml of water? 6. 20ml of a 1.103% w/v calcium lactate solution was analysed by titration against d
1. In a standarisation of hydrochloric acid solution, 0.1232g of sodium carbonate were used. calculate the number of moles of sodium carbonate used. 2. In a standarisation of hydrochloric acid solution, 0.1099g of sodium carbonate were used. This resulted in a titre value of 25.49ml. calculate the number of moles of hydrochlo
Acetylsalicylic acid acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetysalicylic acid. Acetylsalicylic acid has only one acidic hydrogen. What is the molar mass of acetylsalicylic acid? I know the answer but I need help to set up the problem and to k
How does the solubility of a particular reactant affect its ability to raise pH? I am particularly interested in the difference between sodium carbonate and calcium carbonate. Calcium carbonate is much much less soluble than sodium carbonate. However, does the solubility of the carbonate matter when adjusting pH from say
In a lab experiment, a solution of weak acids in water exhibit a pH of 3.7; the solution is known to have a known quantity of dissolved solids in solution. Paper makers alum (aluminum sulfate = Al2(SO4)3) is supposed to be used to coagulate/flocculate the dissolved solids in order to precipitate those solids. In the course
I have a lab experiment in which I have a slurry of wood pulp at a pH of 4.0; I'm asked to use sodium carbonate to raise the pH of the slurry to pH 5.5. I then press the wood slurry to de-water and place it in an oven until it is bone dry. I then take the wood sample out of the oven and place it in a bath of water to determine h
2. Determine the amount of each component recovered and total their masses. Calculate the % recovery based on your starting mass. Amine with watch glass weighed 18.5197g - 18.4998g = 0.0199g, substance was yellow. Carbonoxylic acid with watch glass weighed 18.7402g - 18.7237g = 0.0165g. 3. Calculate the % composition of the mi
1. The half reaction of NpO2+ to Np+4 is a. an acid-base reaction b. a redox reaction c. reduction d. oxidation 2. The standard hydrogen electrode has a half-cell potential of 0.00v. This is due to a. arbitrary convention b. hydrogen gas being insoluble in water c. coincidence d.
1. The following is best described by which type of reaction? CaCO3 --> CaO + CO2 A. decompostion B. acid-base neutralization C. single displacement D. redox E. double-displacement (metathetical) 2. The following best describes which type of reation? 2Ca + O2 --> 2CaO a. decomposition b. acid-base neutraliz
This problem indicates that 1 gram of hydrated boric acid (H3BO3) is added to 1 liter of water at pH 7.0 and at standard temperature. The solubility is stated in the problem as 5.7 grams per 100 ml of solution. A pKa is also given as 9.24. 1) What does the pKa value mean? 2) How would I determine the amount of boric acid
What type of reaction does this describe? metal + H2O --> metal oxide + H2 a. decomposition b. acid-base neutralization c. single displacement d. redox e. double-displacement (metathetical).
The Ksp for Fe(OH)2 is 1.8 x 10-11. Will a precipitate form if an 0.4M solution of FeCl2, has its pH raised to 8.3? What is the solubility of Mg+2 in 0.03M HF? Ka for hydrofluoric acid is 6.6 x 10-4. The Ksp for magnesium fluoride is 3.7 x 10-8 Also: Complete the following reactions: a. H2PO4^- +H^+ ->
Assignment 1 of Procedure 1 1. Calculate the molarity of the freshly-prepared ascorbic acid standard (known strength) solution: (a) Mass of ascorbic acid used:0.05g (b) Moles of ascorbic acid (MW=176.1 g/mol):not sure 0.000284 (c) Total volume of standard solution prepared (mL):100.01mL (d) Asc
40.00 mL of an unknown ammonia solution is titrated with 25.0 mL of 0.105M HCl to the equivalence point. The Kb for ammonia is 1.8 x 10-5. What was the concentration of the original ammonia solution? What is the concentration of NH4Cl at the equivalence point? What is the pH at that point?
What is the pH of a solution containing 0.3M NaC2H3O2 and 0.2M HC2H3O2? The Ka for acetic acid is 1.8 x 10-5.
1. The Ka for HF is 6.6 x 10^-4. What percentage of the HF is ionized if 5 grams are dissolved in 1 liter of water? 2, Assume an indicator, HA, has a Ka od exactly 10^-7. This means that at pH = 7 there are equal numbers of molecules of both colors. What is the ration of colors at pH values of 7.2 and 8.0?
1. The hydration reaction , Na2HPO4 + 2H2O -> Na2HPO4 x 2H2O has a Kp = 6000 at 300K If excess dry, anhydrous Na2HPO4 is added to a 3L container holding 25mmHg of water vapor, what will be the pressure of water after it equilibrates with the sodium phosphate? 2. What is the pH if 2g of NaC2H3O2 and 1g of HC2H3O2 are mixed
My text book lists "ordinary vinegar" as having a pH of 2.4. Using the data from the attached problem find the concentration of acetic acid in vinegar.
1. Which of the following could NOT be a Bronsted-Lowry base? a. HCO3- b. F- c. SO3-2 d. NH4+ 2. What is the pH of a 0.1M HCl solution? a. 0.1 b. 0 c. 1 d. 10 3. Which is the stronger (more highly ionized) acid? a. HF b. HCl c. HBr d. HI 4. Which of
How much NH4Cl must be added to 2.00 liters of 0.200 M aqueous ammonia to give a solution with pH= 8.20? Assume no volume change due to the addition of NH4Cl. a) 246 g b) 166 g c) 2.25 g d) 123 g e) 14.6 g
Calculate the pH for a buffer solution prepared by mixing 100. mL of 0.60 M NH3 and 200. mL of 0.45 M NH4Cl. The Ka of NH4 + = 5.6 x 10^-10. a) 8.65 b) 9.08 c) 9.87 d) 4.90 e) 6.62
The pH of a 0.12 M solution of a weak base is 10.30. What is the value of pKb for this weak base? a.) 3.70 b.) 6.48 c.) 10.30 d.) 5.44 e.) 4.49.